Chemistry 30 Unit C Module 5 Final Assignment
Module 5 Final Assignment
Marks
Maximum
Possible
Earned
%
59
Lesson 1
View the Virtual Investigation on Oxidation States in Module 5 Lesson 1.5 and
use the information to fill in the table in Question 1.
1.
Identify the characteristic colour of the various oxidation states of manganese.
Answer (3 Marks)
Oxidation State
+7
Colour
+6
+4
2. What is disproportionation? Provide an example.
Answer (2 Marks)
Page 1 of 12
Chemistry 30 Unit C Module 5 Final Assignment
Lesson 2
________________________________________________________________
View the Virtual Investigation “Predicting Redox Reactions” in Module 5
Lesson 2.3 and use the results to answer Questions 3 - 7.
3. Predict the products for each system in the Virtual Investigation. Your response
should include:
•
•
•
•
All species initially present
All oxidizing agents and reducing agents. Identify the Strongest Reducing
Agent (SRA) and Strongest Oxidizing Agent (SOA)
If the reaction is spontaneous, indicate “yes” and write the half-reactions
and the balanced net ionic equation. If the reaction is non-spontaneous,
simply indicate “no” in the blank . Include the half-reactions but it is not
necessary to write net ionic equation if the reaction is non-spontaneous.
System 1 and 2 have been completed for you as examples. Refer to
these examples before completing the rest of the System tables –
they will be very helpful in clarifying common mistakes!
System 1 Example – liquid water and solid calcium
Species List
H2O(l), Ca(s)
Oxidizing agents
H2O(l)
SOA= H2O(l)
Reducing agents
H2O(l), Ca(s)
SRA= Ca(s)
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
Yes
2 H2O(l) + 2e- → H2(g) + 2 OH-(aq)
Ca(s) →Ca2+(aq) + 2e2 H2O(l) + Ca(s) →Ca2+(aq) + H2(g) + 2 OH-(aq)
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Chemistry 30 Unit C Module 5 Final Assignment
System 2 Example – aqueous hydrochloric acid and solid silver
metal
Species List
H+(aq), Cl-(aq), H2O(l), Ag(s)
Oxidizing agents
H2O(l), H+(aq)
SOA= H+(aq)
Reducing agents
H2O(l), Ag(s), Cl-(aq), Cl-(aq) + H2O(l),
SRA= Ag(s)
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
No
2 H+(aq) + 2e- → H2(g)
Ag(s) → Ag1+(aq) + 1eNon-spontaneous
System 3 – aqueous hydrochloric acid and solid magnesium metal
Answer (4 Marks)
Species List
Oxidizing Agents
Reducing agents
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
Page 3 of 12
Chemistry 30 Unit C Module 5 Final Assignment
System 4 – Acidified aqueous iron(II) nitrate and aqueous potassium
dichromate
Hint: Study the species list carefully and remember to consider combination
agents!
Answer (4 Marks)
Species List
Oxidizing agents
Reducing agents
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
System 5 – aqueous hydrogen peroxide and aqueous iron(III) nitrate
Hint: This system is not acidified.
Answer (4 Marks)
Species List
Oxidizing Agents
Reducing agents
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
Page 4 of 12
Chemistry 30 Unit C Module 5 Final Assignment
System 6 – aqueous zinc nitrate and aqueous chromium(II) chloride
Answer (4 Marks)
Species List
Oxidizing agents
Reducing agents
Spontaneous?
Reduction halfReaction
Oxidation halfreaction
Net ionic equation
System 7 – aqueous silver nitrate and solid copper metal
Answer (4 Marks)
Species List
Oxidizing agents
Reducing agents
Spontaneous?
Reduction halfreaction
Oxidation halfreaction
Net ionic equation
Page 5 of 12
Chemistry 30 Unit C Module 5 Final Assignment
4. Record your observations from the Virtual Investigation in the following table.
Answer (5 Marks)
System
Observable Evidence of a Spontaneous Reaction
1.
Bubbling
Disintegration of the solid metal
pH increases.
2.
No observable changes
3.
4.
5.
6.
7.
5. Describe the diagnostic test that could be used to identify the gas produced in
System 1.
Your response should include
• a description of how the test is performed
• identity of the gas being tested for
• the results of the test
Hint: See page 805 in your textbook for a list of diagnostic tests.
Answer (3 Marks)
Page 6 of 12
Chemistry 30 Unit C Module 5 Final Assignment
6. Describe the diagnostic test that could be used to identify the gas produced in
System 5.
Your response should include
• a description of how the test is performed
• identity of the gas being tested for
• the results of the test
Hint: See page 805 in your textbook for a list of diagnostic tests.
Answer (3 Marks)
7. Measuring pH change is sometimes used as a diagnostic test. In which
systems might we have used pH change as evidence of a spontaneous
reaction? Explain your reasoning.
Answer (2 Marks)
Page 7 of 12
Chemistry 30 Unit C Module 5 Final Assignment
Lesson 3
Perform the Virtual Investigation “Redox Titration, Exercise 1, Procedures 1
and 2” in Module 5 Lesson 3.2 and use the results to answer Questions 8 – 16.
8. Fill in the data table below with the data you collected from Part 1 of Experiment
1 (coarse titration using the NEW hydrogen peroxide). Remember, a burette
measures the volume dispensed.
Answer (1 Mark)
Volume of KMnO4 added (coarse titration)
Initial Burette reading
(mL)
Final Burette Reading
(mL)
Volume of KMnO4 used
(mL)
Page 8 of 12
Chemistry 30 Unit C Module 5 Final Assignment
9. Fill in the data table below with the data you collected from Part 2 of Experiment
1 (fine titration using the NEW hydrogen peroxide).
Answer (3 Marks)
Volume of KMnO4 added (fine titration) - Record the data from the three
most consistent trials.
Initial Burette
reading (mL)
Final Burette
Reading (mL)
Volume of
KMnO4 used
(mL)
Average
volume of
KMnO4 used
(mL)
Trial 1
Trial 2
Trial 3
10. Calculate the concentration of the NEW hydrogen peroxide, following the steps
below. Use your answer from Question 26 as the titrant volume.
Answer (4 Marks)
Write the halfreactions and
net redox
reaction
(remember KMnO4
dissociates into K+ and
MnO4-)
Calculate
moles of MnO4added from the
average
volume of
KMnO4 used
Calculate
moles of NEW
H2O2
Calculate
concentration
of NEW H2O2
Page 9 of 12
Chemistry 30 Unit C Module 5 Final Assignment
11. Use your answer for the concentration of NEW H2O2 above and Table 1 on p.
603 in your textbook to estimate the percentage by volume concentration of the
NEW hydrogen peroxide solution. (No calculation is needed here.)
Answer (1 Mark)
12. Fill in the data table below with the data you collected from Part 1 of Experiment
1 (coarse titration using the OLD hydrogen peroxide).
Answer (2 Marks)
Volume of KMnO4 added (coarse titration)
Initial Burette reading
(mL)
Final Burette Reading
(mL)
Volume of KMnO4 used
(mL)
Page 10 of 12
Chemistry 30 Unit C Module 5 Final Assignment
13. Fill in the data table below with the data you collected from Part 2 of Experiment
1 (fine titration using the OLD hydrogen peroxide).
Answer (3 Marks)
Volume of KMnO4 added (fine titration)
Trial 1
Initial Burette reading
(mL)
Final Burette Reading
(mL)
Volume of KMnO4 used
(mL)
Average volume of
KMnO4 used (mL)
Trial 2
Trial 3
14. Calculate the concentration of the OLD hydrogen peroxide, following the steps
below. Use your answer from #31 as the titrant volume.
Answer (4 Marks)
Write the halfreactions and
net redox
reaction
Calculate
moles of
MnO4Calculate
moles of OLD
H2O2
Calculate
concentration
of OLD H2O2
Page 11 of 12
Chemistry 30 Unit C Module 5 Final Assignment
15. Use your calculated concentration of OLD H2O2 and Table 1 on p. 603 in your
textbook to estimate the percentage by volume concentration of the OLD
hydrogen peroxide solution. (No calculation is needed here.)
Answer (1 Mark)
16. Compare your results for the concentration of the NEW hydrogen peroxide to
the concentration of the OLD hydrogen peroxide. Based on the properties of
hydrogen peroxide, explain any difference that you notice between the NEW
and OLD samples
Answer (2 Marks)
Page 12 of 12